We’re being asked to calculate the lattice energy of rubidium chloride (RbCl).
Recall that lattice energy is the energy required to combine two gaseous ions into a solid ionic compound:
Mx+(g) + Ny–(g) → MyNx(s)
To calculate for lattice energy, we need to do the Born-Haber cycle for RbCl.
We start with the corresponding formation equation for RbCl:
Rb(s) + 1/2 Cl2(g) → RbCl(s), ΔH˚f
The enthalpy of formation (ΔHf) of rubidium chloride is -430.5 kJ/mol. The enthalpy of sublimation for rubidium is 86 kJ/mol, and the first ionization energy of rubidium is 402 kJ/mol. The bond dissociation energy of (g) is 243 kJ/mol, and the electron affinity of chlorine is -349 kJ/mol. Calculate the lattice energy of RbCl (s), in kJ/mol.
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What scientific concept do you need to know in order to solve this problem?
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